Atomic Structure Matter is anything that occupies space
- Slides: 26
Atomic Structure
Matter is anything that occupies space
Composition of Matter is composed of particles, which may be atoms, molecules or ions
Law of Conservation of Mass The law of conservation of mass states that matter is neither created nor destroyed in the course of a chemical reaction.
Scientists that led to the modern view of the atom? • Dalton • Crooke • Stoney • Thomson • Millikan • Rutherford • Bohr • Chadwick
Dalton’s Atomic Theory The law of conservation of mass states that matter is neither created nor destroyed in the course of a chemical reaction. Dalton proposed that all matter was composed of atoms, indivisible and indestructible building blocks. While all atoms of an element were identical, different elements had atoms of differing size and mass. Dalton stated that all compounds were composed of combinations of these atoms in defined ratios. Dalton also postulated that chemical reactions resulted in the rearrangement of the reacting atoms.
William Crooke discovered cathode rays and found evidence that these cathode rays were actually particles
J J Thomson discovered that electrons had negative charge. He calculated the e/m for electrons.
J J Thomson proposed that atoms consist of small negative electrons embedded in a massive positive sphere
George Stoney proposed the name of ‘electron’ for the negatively charged particles
Cathode Rays Streams of negatively charged particles (electrons) that travel from the cathode to the anode a vacuum tube.
Robert Millikan Determined the size of the charge on the electron using the oil drop experiment.
Ernest Rutherford discovered the nucleus of the atom by bombarding gold foil with alpha particles and the scattering indicated a hard-dense core in the centre of the atom. Rutherford bombarded different elements and found that they all gave out the same positively charged particle which was identical to the nucleus of the hydrogen atom. He called this particle the proton
Niels Bohr proposed that the electrons in atoms were arranged in a series of concentric circular orbits at an increasing distance from the nucleus
James Chadwick brought about the release of neutral particles with the same mass as the proton by bombarding sample of beryllium with alpha particles. He named them neutrons.
Atom Smallest particle of matter that can take part in a chemical reaction
Properties of Sub atomic Particles Particle Relative Charge Relative Mass Location Neutron 0 1 Nucleus Proton +1 1 Nucleus Electron -1 1/1838 Shells
Atomic Number of Protons in Atom
Mass Number of protons and neutrons in an atom
Isotopes Atoms with the same atomic number but different mass number due to the different number of neutrons in the nucleus
Isotopes of Hydrogen
Isotopes of Carbon
Relative Atomic Mass Is the average mass of the isotopes of an element as they occur in nature taken abundances into account when compared to one twelfth of the mass of the 12 C atom
Mass Spectrometer Principle Positively charged ions are separated on the basis of their relative masses as they move in a magnetic field
Processes in Mass Spectrometer Processes 1. Vaporisation 2. Ionisation 3. Acceleration 4. Separation 5. Detection
Uses of Mass Spectrometer Uses Identify compounds e. g. 1. in analysis of gases from waste dumps 2. in trace organic pollutants in water 3. in drug testing Measure relative atomic mass Measure relative abundance of isotopes
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